An unknown amount of helium (He) gas occupies 10.5 L at 1.47 atm pressure and 321 K. What is the mass of helium gas in the container?
Use R = 0.0821 L.atm/(mol.K).
____________ g He. Do NOT enter unit. Report your final answer with 3 SFs.
Use PV = nRT and solve for n = number of mole He.
Then mol He x molar mass He = grams He. Remember to use T in kelvin.
degrees L = degrees C + 273 = ?
Post your work if you get stuck.
To calculate the mass of helium gas in the container, we'll use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L.atm/(mol.K))
T = temperature (in Kelvin)
First, let's convert the given temperature from Celsius to Kelvin by adding 273.15 K:
T = 321 K
Now, let's rearrange the equation to solve for the number of moles of gas (n):
n = PV / RT
Substituting the given values into the equation:
n = (1.47 atm * 10.5 L) / (0.0821 L.atm/(mol.K) * 321 K)
Calculating the expression:
n ≈ 0.541 mol
Now, to find the mass of helium gas, we need to multiply the number of moles (n) by the molar mass of helium (He). The molar mass of helium is approximately 4.003 grams/mol.
m = n * molar mass
m = 0.541 mol * 4.003 g/mol
Calculating the expression:
m ≈ 2.166 g
Therefore, the mass of helium gas in the container is approximately 2.166 g.
I am just entering the numbers in the right column so you will know where I got numbers from.
V = 10.5
P = 1.47
T = 321 K
R = 0.0821
M = 4.003g/mol
Here's the work,, Let me know if I did anything wrong.
N = P1 V1 / RT1 =
(1.47atm)(10.5) = 15.435 / (0.0821) (321) = 26.3541
15.435 / 26.3541 = 0.58567
m = n x m
= (0.58567mol) (4.003g/mol) = 2.34444
Correct answer is 2.34
Am I right @DrBob222?